A buffer contains equal amounts of a weak acid and its conjugate base and has a pH of 5.25. How will the concentration of the weak acid in the buffer change after the addition of a small amount of strong base?

A buffer solution is prepared by adding 9.04 mL of 1.27 M HBr to 190.0 mL of 0.11 M methylamine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong base is added. What is the pH of the resulting solution? Round your answer to 2 decimal places.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.150 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10^-4.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HF is 3.5 × 10⁻⁴.

A benzoate buffer is prepared containing 0.33 M benzoic acid and 0.28 M benzoate. The Ka of benzoic acid is 6.3 x 10^-5. What is the pH of the buffer after the addition of 20 mL of 0.50 M NaOH to 100 mL of this buffer?

A buffer contains the weak acid HA and its conjugate base A⁻. The weak acid has a pKa of 5.25 and the buffer has a pH of 4.82. Which statement is true of the relative concentrations of the weak acid and the conjugate base in the buffer?

A buffer solution is made by dissolving 0.780 moles of NaClO in 1.00 L of 0.560 M HClO. What is the pH of the solution after 0.140 moles of NaOH is added? The Ka of HClO is 2.9 × 10^-8.

Calculate the pH value for a buffer solution prepared by adding 1.0 mL of a 0.10M acetic acid solution to 20 mL of a 0.10M sodium acetate solution. (Ka = 1.7 × 10⁻⁵)

If you have 500.0 mL of a 0.10 M solution of HClO, what mass of NaClO (molar mass = 74.44 g/mol) do you need to add to make a buffer with a pH of 7.5?